Question

Consider the following equilibrium:

Answer 1

Answer : The wrong equation is, $K_p=K_c\times (RT)^{-5}$

Explanation :

The given equilibrium reaction is,

$4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)$

The expression for equilibrium constant in terms of concentration,

$K_c=\frac{1}{[O_2]^3}\\\\K_c=[O_2]^{-3}$

The expression for equilibrium constant in terms of pressure,

$K_p=\frac{1}{(P_{O_2})^3}\\\\K_p=(P_{O_2})^{-3}$

The relation between the equilibrium constant in terms of concentration and equilibrium constant in terms of pressure will be,

$K_p=K_c\times (RT)^{\Delta n_g}$

where,

$\Delta n_g$= number of moles of gaseous products - number of moles of gaseous reactants

R = gas constant

T= temperature

For reaction the given reaction,

$\Delta n_g$= number of moles of gaseous products - number of moles of gaseous reactants= 0 - 3 = -3

$K_p=K_c\times (RT)^{-3}$

Therefore, the correct equations for equilibrium are, $K_c=[O_2]^{-3}$, $K_p=(P_{O_2})^{-3}$ and $K_p=K_c\times (RT)^{-3}$

Answer 2

L think the answer is kc=:02:-3